0620_w08_qp_03

1. Location Entry Codes
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2. This document consists of 12 printed pages.
IB08 11_0620_31/6RP
© UCLES 2008 [Turn over
*2942397288*
For Examiner's Use
1
2
3
4
5
6
7
Total
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS
International General Certificate of Secondary Education
CHEMISTRY 0620/31
Paper 3 (Extended) October/November 2008
1 hour 15 minutes
Candidates answer on the Question Paper.
No Additional Materials are required.
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use a pencil for any diagrams, graphs or rough working.
Do not use staples, paper clips, highlighters, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES
Answer all questions.
A copy of the Periodic Table is printed on page 12.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part
questions.
First Variant Question Paper

3. 2
© UCLES 2008 0620/31/O/N/08
For
Examiner's
Use
1 Complete the following table.
gas test for gas
ammonia
bleaches damp litmus paper
hydrogen
relights a glowing splint
turns limewater milky
[Total: 5]

4. 3
© UCLES 2008 0620/31/O/N/08 [Turn over
For
Examiner's
Use
2 There are three types of giant structure – ionic, metallic and macromolecular.
(a) Sodium nitride is an ionic compound. Draw a diagram that shows the formula of the
compound, the charges on the ions and the arrangement of the valency electrons
around the negative ion.
Use x to represent an electron from a sodium atom.
Use o to represent an electron from a nitrogen atom.
[3]
(b) (i) Describe metallic bonding.
[3]
(ii) Use the above ideas to explain why
metals are good conductors of electricity,
[1]
metals are malleable.
[2]
(c) Silicon(IV) oxide has a macromolecular structure.
(i) Describe the structure of silicon(IV) oxide (a diagram is not acceptable).
[3]
(ii) Diamond has a similar structure and consequently similar properties.
Give two physical properties common to both diamond and silicon(IV) oxide.
[2]
[Total: 14]

5. 4
© UCLES 2008 0620/31/O/N/08
For
Examiner's
Use
3 Steel is an alloy made from impure iron.
(a) Both iron and steel rust. The formula for rust is Fe2O3.2H2O.
It is hydrated iron(III) oxide.
(i) Name the two substances that must be present for rusting to occur.
[2]
(ii) Painting and coating with grease are two methods of preventing iron or steel from
rusting. Give two other methods.
[2]
(b) (i) Name a reagent that can reduce iron(III) oxide to iron.
[1]
(ii) Write a symbol equation for the reduction of iron(III) oxide, Fe2O3, to iron.
[2]
(c) (i) Calculate the mass of one mole of Fe2O3.2H2O.
[1]
(ii) Use your answer to (i) to calculate the percentage of iron in rust.
[2]
(d) Iron from the blast furnace is impure. Two of the impurities are carbon and silicon.
These are removed by blowing oxygen through the molten iron and adding calcium
oxide.
(i) Explain how the addition of oxygen removes carbon.
[1]
(ii) Explain how the addition of oxygen and calcium oxide removes silicon.
[2]
[Total: 13]

6. 5
© UCLES 2008 0620/31/O/N/08 [Turn over
For
Examiner's
Use
4 Across the world, food safety agencies are investigating the presence of minute traces of
the toxic hydrocarbon, benzene, in soft drinks. It is formed by the reduction of sodium
benzoate by vitamin C.
INGREDIENTS
Orange juice,
sodium benzoate,
vitamin C
(a) Sodium benzoate is a salt, it has the formula C6H5COONa. It can be made by the
neutralisation of benzoic acid by sodium hydroxide.
(i) Deduce the formula of benzoic acid.
[1]
(ii) Write a word equation for the reaction between benzoic acid and sodium hydroxide.
[1]
(iii) Name two other compounds that would react with benzoic acid to form
sodium benzoate.
[2]
(b) Benzene contains 92.3% of carbon and its relative molecular mass is 78.
(i) What is the percentage of hydrogen in benzene?
[1]
(ii) Calculate the ratio of moles of C atoms: moles of H atoms in benzene.
[2]
(iii) Calculate its empirical formula and then its molecular formula.
The empirical formula of benzene is
The molecular formula of benzene is [2]

7. 6
© UCLES 2008 0620/31/O/N/08
For
Examiner's
Use
(c) The structural formula of Vitamin C is drawn below.
CC
CO C C C
OH H
HH H
OH
O
HO OH
(i) What is its molecular formula?
[1]
(ii) Name the two functional groups which are circled.
[2]
[Total: 12]

8. 7
© UCLES 2008 0620/31/O/N/08 [Turn over
For
Examiner's
Use
5 The electrolysis of concentrated aqueous sodium chloride produces three commercially
important chemicals hydrogen, chlorine and sodium hydroxide.
(a) The ions present are Na+
(aq), H+
(aq) ,Cl–
(aq) and OH–
(aq).
(i) Complete the ionic equation for the reaction at the negative electrode (cathode).
+ H2 [1]
(ii) Complete the ionic equation for the reaction at the positive electrode (anode).
− Cl2 [1]
(iii) Explain why the solution changes from sodium chloride to sodium hydroxide.
[1]
(b) (i) Why does the water supply industry use chlorine?
[1]
(ii) Name an important chemical that is made from hydrogen.
[1]
(iii) How is sodium hydroxide used to make soap?
[2]
[Total: 7]

9. 8
© UCLES 2008 0620/31/O/N/08
For
Examiner's
Use
6 The reactivity series lists metals in order of reactivity.
(a) To find out which is the more reactive metal, zinc or tin, the following experiment could
be carried out.
tin(II) nitrate(aq)
piece of zinc
shiny surface
piece of zinc,
surface still shiny
NO REACTION (NR)
surface of zinc covered
with a grey deposit
REACTION (R)
This experiment could be carried out with other metals and the results recorded in a
table. Then the order of reactivity can be deduced.
(i) The order was found to be:
manganese most reactive
zinc
tin
silver least reactive
Complete the table of results from which this order was determined.
aqueous
solution
tin
Sn
manganese
Mn
silver
Ag
zinc
Zn
tin(II) nitrate R NR R
manganese(II) nitrate
silver(I) nitrate
zinc nitrate
[3]
(ii) Write the ionic equation for the reaction between tin atoms and silver(I) ions.
[2]

10. 9
© UCLES 2008 0620/31/O/N/08 [Turn over
For
Examiner's
Use
(iii) The following is a redox reaction.
Mn + Sn2+
Mn2+
+ Sn
Indicate on the equation the change which is oxidation.
Give a reason for your choice.
[2]
(iv) Explain why experiments of this type cannot be used to find the position of
aluminium in the reactivity series.
[2]
(b) Potassium and calcium are very reactive metals at the top of the series. Because their
ions have different charges, K+
and Ca2+
, their compounds behave differently when
heated.
(i) Explain why the ions have different charges.
[2]
(ii) Their hydroxides are heated.
If the compound decomposes, complete the word equation.
If it does not decompose, write “no reaction”.
Potassium hydroxide
Calcium hydroxide [2]
(iii) Complete the equations for the decomposition of their nitrates.
2KNO3 +
2Ca(NO3)2 + + [4]
[Total: 17]

11. 10
© UCLES 2008 0620/31/O/N/08
For
Examiner's
Use
7 The alkanes are generally unreactive. Their reactions include combustion, substitution and
cracking.
(a) The complete combustion of an alkane gives carbon dioxide and water.
(i) 10 cm3
of butane is mixed with 100 cm3
of oxygen, which is an excess. The mixture
is ignited. What is the volume of unreacted oxygen left and what is the volume of
carbon dioxide formed?
C4H10(g) + (g)O6 22
1
4CO2(g) + 5H2O(l)
Volume of oxygen left = cm3
Volume of carbon dioxide formed = cm3
[2]
(ii) Why is the incomplete combustion of any alkane dangerous, particularly in an
enclosed space?
[2]
(b) The equation for a substitution reaction of butane is given below.
CH3−CH2−CH2−CH3 + Cl2 CH3−CH2−CH2−CH2 −Cl + HCl
(i) Name the organic product.
[1]
(ii) This reaction does not need increased temperature or pressure.
What is the essential reaction condition?
[1]
(iii) Write a different equation for a substitution reaction between butane and chlorine.
[1]

12. 11
© UCLES 2008 0620/31/O/N/08
For
Examiner's
Use
(c) Alkenes are more reactive and industrially more useful than alkanes.
They are made by cracking alkanes.
C7H16 CH3−CH=CH2 + CH3−CH2−CH=CH2 + H2
heptane propene but−1−ene
(i) Draw the structural formula of the polymer poly(propene).
[2]
(ii) Give the structural formula and name of the alcohol formed when but-1-ene reacts
with steam.
name [1]
structural formula
[1]
(iii) Deduce the structural formula of the product formed when propene reacts with
hydrogen chloride.
[1]
[Total: 12]

13. 12
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of
Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
© UCLES 2008 0620/31/O/N/08
Group
140
Ce
Cerium
58
141
Pr
Praseodymium
59
144
Nd
Neodymium
60
Pm
Promethium
61
150
Sm
Samarium
62
152
Eu
Europium
63
157
Gd
Gadolinium
64
159
Tb
Terbium
65
162
Dy
Dysprosium
66
165
Ho
Holmium
67
167
Er
Erbium
68
169
Tm
Thulium
69
173
Yb
Ytterbium
70
175
Lu
Lutetium
71
232
Th
Thorium
90
Pa
Protactinium
91
238
U
Uranium
92
Np
Neptunium
93
Pu
Plutonium
94
Am
Americium
95
Cm
Curium
96
Bk
Berkelium
97
Cf
Californium
98
Es
Einsteinium
99
Fm
Fermium
100
Md
Mendelevium
101
No
Nobelium
102
Lr
Lawrencium
103
1
H
Hydrogen
1
7
Li
Lithium
3
23
Na
Sodium
11
24
Mg
Magnesium
12
40
Ca
Calcium
20
45
Sc
Scandium
21
48
Ti
Titanium
22
51
V
Vanadium
23
52
Cr
Chromium
24
55
Mn
Manganese
25
56
Fe
Iron
26
59
Co
Cobalt
27
59
Ni
Nickel
28
64
Cu
Copper
29
65
Zn
Zinc
30
70
Ga
Gallium
31
27
Al
Aluminium
13
11
B
Boron
5
12
C
Carbon
6
14
N
Nitrogen
7
16
O
Oxygen
8
19
F
Fluorine
9
28
Si
Silicon
14
31
P
Phosphorus
15
32
S
Sulphur
16
35.5
Cl
Chlorine
17
40
Ar
Argon
18
20
Ne
Neon
10
4
He
Helium
2
73
Ge
Germanium
32
75
As
Arsenic
33
79
Se
Selenium
34
80
Br
Bromine
35
84
Kr
Krypton
36
39
K
Potassium
19
88
Sr
Strontium
38
89
Y
Yttrium
39
91
Zr
Zirconium
40
93
Nb
Niobium
41
96
Mo
Molybdenum
42
Tc
Technetium
43
101
Ru
Ruthenium
44
103
Rh
Rhodium
45
106
Pd
Palladium
46
108
Ag
Silver
47
112
Cd
Cadmium
48
115
In
Indium
49
119
Sn
Tin
50
122
Sb
Antimony
51
128
Te
Tellurium
52
127
I
Iodine
53
131
Xe
Xenon
54
137
Ba
Barium
56
139
La
Lanthanum
57*
178
Hf
Hafnium
72
181
Ta
Tantalum
73
184
W
Tungsten
74
186
Re
Rhenium
75
190
Os
Osmium
76
192
Ir
Iridium
77
195
Pt
Platinum
78
197
Au
Gold
79
201
Hg
Mercury
80
204
Tl
Thallium
81
207
Pb
Lead
82
209
Bi
Bismuth
83
Po
Polonium
84
At
Astatine
85
Rn
Radon
86
Fr
Francium
87
227
Ac
Actinium
89
9
Be
Beryllium
4
IIIIIIIVVVIVII0
85
Rb
Rubidium
37
133
Cs
Caesium
55
226
Ra
Radium
88
Thevolumeofonemoleofanygasis24dm3atroomtemperatureandpressure(r.t.p.).
a
X
b
a=relativeatomicmass
X=atomicsymbol
b=proton(atomic)number
Key
*58-71Lanthanoidseries
90-103Actinoidseries
DATASHEET
ThePeriodicTableoftheElements

14. This document consists of 12 printed pages.
IB08 11_0620_03_TZ/4RP
© UCLES 2008 [Turn over
*7507316830*
For Examiner's Use
1
2
3
4
5
6
7
Total
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS
International General Certificate of Secondary Education
CHEMISTRY 0620/32
Paper 3 (Extended) October/November 2008
1 hour 15 minutes
Candidates answer on the Question Paper.
No Additional Materials are required.
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use a pencil for any diagrams, graphs or rough working.
Do not use staples, paper clips, highlighters, glue or correction fluid.
DO NOT WRITE IN ANY BARCODES
Answer all questions.
A copy of the Periodic Table is printed on page 12.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part
questions.
Second Variant Question Paper

15. 2
© UCLES 2008 0620/32/O/N/08
For
Examiner's
Use
1 Complete the following table.
gas test for gas
turns damp red litmus paper blue
bleaches damp litmus paper
hydrogen
oxygen
carbon dioxide
[Total: 5]

16. 3
© UCLES 2008 0620/32/O/N/08 [Turn over
For
Examiner's
Use
2 There are three types of giant structure – ionic, metallic and macromolecular.
(a) Sodium sulphide is an ionic compound. Draw a diagram that shows the formula of the
compound, the charges on the ions and the arrangement of the valency electrons
around the negative ion.
Use x to represent an electron from a sodium atom.
Use o to represent an electron from a sulphur atom.
[3]
(b) (i) Describe metallic bonding.
[3]
(ii) Use the above ideas to explain why
metals are good conductors of electricity,
[1]
metals are malleable.
[2]
(c) Silicon(IV) oxide has a macromolecular structure.
(i) Describe the structure of silicon(IV) oxide (a diagram is not acceptable).
[3]
(ii) Diamond has a similar structure and consequently similar properties.
Give two physical properties common to both diamond and silicon(IV) oxide.
[2]
[Total: 14]

17. 4
© UCLES 2008 0620/32/O/N/08
For
Examiner's
Use
3 Steel is an alloy made from impure iron.
(a) Both iron and steel rust. The formula for rust is Fe2O3.2H2O.
It is hydrated iron(III) oxide.
(i) Name the two substances that must be present for rusting to occur.
and [2]
(ii) Painting and coating with grease are two methods of preventing iron or steel from
rusting. Give two other methods.
[2]
(b) (i) Name a reagent that can reduce iron(III) oxide to iron.
[1]
(ii) Write a symbol equation for the reduction of iron(III) oxide, Fe2O3, to iron.
[2]
(c) (i) Calculate the mass of one mole of Fe2O3.2H2O.
[1]
(ii) Use your answer to (i) to calculate the percentage of water in rust.
[2]
(d) Iron from the blast furnace is impure. Two of the impurities are carbon and silicon.
These are removed by blowing oxygen through the molten iron and adding calcium
oxide.
(i) Explain how the addition of oxygen removes carbon.
[1]
(ii) Explain how the addition of oxygen and calcium oxide removes silicon.
[2]
[Total: 13]

18. 5
© UCLES 2008 0620/32/O/N/08 [Turn over
For
Examiner's
Use
4 Across the world, food safety agencies are investigating the presence of minute traces of
the toxic hydrocarbon, benzene, in soft drinks. It is formed by the reduction of sodium
benzoate by vitamin C.
INGREDIENTS
Orange juice,
sodium benzoate,
vitamin C
(a) Sodium benzoate is a salt, it has the formula C6H5COONa. It can be made by the
neutralisation of benzoic acid by sodium hydroxide.
(i) Deduce the formula of benzoic acid.
[1]
(ii) Write a word equation for the reaction between benzoic acid and sodium hydroxide.
[1]
(iii) Name two other compounds that would react with benzoic acid to form
sodium benzoate.
[2]

19. 6
© UCLES 2008 0620/32/O/N/08
For
Examiner's
Use
(b) Benzene contains 92.3% of carbon and its relative molecular mass is 78.
(i) What is the percentage of hydrogen in benzene?
[1]
(ii) Calculate the ratio of moles of C atoms: moles of H atoms in benzene.
[2]
(iii) Calculate its empirical formula and then its molecular formula.
The empirical formula of benzene is
The molecular formula of benzene is [2]
(c) The structural formula of Vitamin C is drawn below.
CC
CO C C C
OH H
HH H
OH
O
HO OH
(i) What is its molecular formula?
[1]
(ii) Name the two functional groups which are circled.
[2]
[Total: 12]

20. 7
© UCLES 2008 0620/32/O/N/08 [Turn over
For
Examiner's
Use
5 The electrolysis of concentrated aqueous sodium chloride produces three commercially
important chemicals; hydrogen, chlorine and sodium hydroxide.
(a) The ions present are Na+
(aq), H+
(aq) ,Cl –
(aq) and OH–
(aq).
(i) Complete the ionic equation for the reaction at the negative electrode (cathode).
+ H2 [1]
(ii) Complete the ionic equation for the reaction at the positive electrode (anode).
2Cl –
− [1]
(iii) Explain why the solution changes from sodium chloride to sodium hydroxide.
[1]
(b) (i) Why does the water supply industry use chlorine?
[1]
(ii) Name an important chemical that is made from hydrogen.
[1]
(iii) Sodium hydroxide reacts with fats to make soap and glycerine
What type of compound are fats?
[1]
What type of the reaction is this?
[1]
[Total : 7]

21. 8
© UCLES 2008 0620/32/O/N/08
For
Examiner's
Use
6 The reactivity series lists metals in order of reactivity.
(a) To find out which is the more reactive metal, zinc or tin, the following experiment could
be carried out.
tin(II) nitrate(aq)
piece of zinc
shiny surface
piece of zinc,
surface still shiny
NO REACTION (NR)
surface of zinc covered
with a grey deposit
REACTION (R)
This experiment could be carried out with other metals and the results recorded in a
table. Then the order of reactivity can be deduced.
(i) The order was found to be:
manganese most reactive
zinc
tin
silver least reactive
Complete the table of results from which this order was determined.
aqueous
solution
tin
Sn
manganese
Mn
silver
Ag
zinc
Zn
tin(II) nitrate R NR R
manganese(II) nitrate
silver(I) nitrate
zinc nitrate
[3]
(ii) Write the equation for the reaction between zinc and silver(I) nitrate.
[2]

22. 9
© UCLES 2008 0620/32/O/N/08 [Turn over
For
Examiner's
Use
(iii) The following is a redox reaction.
Mn + Sn2+
Mn2+
+ Sn
Indicate on the equation which reagent is the oxidant or oxidizing agent.
Give a reason for your choice.
[2]
(iv) Explain why experiments of this type cannot be used to find the position of
aluminium in the reactivity series.
[2]
(b) Potassium and calcium are very reactive metals at the top of the series. Because their
ions have different charges, K+
and Ca2+
, their compounds behave differently when
heated.
(i) Explain why the ions have different charges.
[2]
(ii) Their hydroxides are heated.
If the compound decomposes, complete the word equation.
If it does not decompose, write “no reaction”.
Potassium hydroxide
Calcium hydroxide [2]
(iii) Complete the equations for the decomposition of their nitrates.
2KNO3 +
2Ca(NO3)2 + + [4]
[Total: 17]

23. 10
© UCLES 2008 0620/32/O/N/08
For
Examiner's
Use
7 The alkanes are generally unreactive. Their reactions include combustion, substitution and
cracking.
(a) The complete combustion of an alkane gives carbon dioxide and water.
(i) 20cm3
of butane is mixed with 150cm3
of oxygen, which is an excess. The mixture
is ignited. What is the volume of unreacted oxygen left and what is the volume of
carbon dioxide formed?
C4H10(g) + 6 1
2
O2 (g) 4CO2(g) + 5H2O (l)
Volume of oxygen left = cm3
Volume of carbon dioxide formed = cm3
[2]
(ii) Why is the incomplete combustion of any alkane dangerous, particularly in an
enclosed space?
[2]
(b) The equation for a substitution reaction of butane is given below.
CH3−CH2−CH2−CH3 + Cl2 CH3−CH2−CH2−CH2 −Cl + HCl
(i) Name the organic product.
[1]
(ii) This reaction does not need increased temperature or pressure.
What is the essential reaction condition?
[1]
(iii) Write a different equation for a substitution reaction between butane and chlorine.
[1]

24. 11
© UCLES 2008 0620/32/O/N/08 [Turn over
For
Examiner's
Use
(c) Alkenes are more reactive and industrially more useful than alkanes.
They are made by cracking alkanes.
C7H16 CH3−CH=CH2 + CH3−CH2−CH=CH2 + H2
heptane propene but−1−ene
(i) Draw the structural formula of the polymer poly(propene).
[2]
(ii) Give the structural formula and name of the alcohol formed when propene reacts
with steam.
name [1]
structural formula
[1]
(iii) Deduce the structural formula of the product formed when but−1−ene reacts with
hydrogen chloride.
[1]
[Total: 12]

25. 12
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of
Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.
© UCLES 2008 0620/32/O/N/08
Group
140
Ce
Cerium
58
141
Pr
Praseodymium
59
144
Nd
Neodymium
60
Pm
Promethium
61
150
Sm
Samarium
62
152
Eu
Europium
63
157
Gd
Gadolinium
64
159
Tb
Terbium
65
162
Dy
Dysprosium
66
165
Ho
Holmium
67
167
Er
Erbium
68
169
Tm
Thulium
69
173
Yb
Ytterbium
70
175
Lu
Lutetium
71
232
Th
Thorium
90
Pa
Protactinium
91
238
U
Uranium
92
Np
Neptunium
93
Pu
Plutonium
94
Am
Americium
95
Cm
Curium
96
Bk
Berkelium
97
Cf
Californium
98
Es
Einsteinium
99
Fm
Fermium
100
Md
Mendelevium
101
No
Nobelium
102
Lr
Lawrencium
103
1
H
Hydrogen
1
7
Li
Lithium
3
23
Na
Sodium
11
24
Mg
Magnesium
12
40
Ca
Calcium
20
45
Sc
Scandium
21
48
Ti
Titanium
22
51
V
Vanadium
23
52
Cr
Chromium
24
55
Mn
Manganese
25
56
Fe
Iron
26
59
Co
Cobalt
27
59
Ni
Nickel
28
64
Cu
Copper
29
65
Zn
Zinc
30
70
Ga
Gallium
31
27
Al
Aluminium
13
11
B
Boron
5
12
C
Carbon
6
14
N
Nitrogen
7
16
O
Oxygen
8
19
F
Fluorine
9
28
Si
Silicon
14
31
P
Phosphorus
15
32
S
Sulphur
16
35.5
Cl
Chlorine
17
40
Ar
Argon
18
20
Ne
Neon
10
4
He
Helium
2
73
Ge
Germanium
32
75
As
Arsenic
33
79
Se
Selenium
34
80
Br
Bromine
35
84
Kr
Krypton
36
39
K
Potassium
19
88
Sr
Strontium
38
89
Y
Yttrium
39
91
Zr
Zirconium
40
93
Nb
Niobium
41
96
Mo
Molybdenum
42
Tc
Technetium
43
101
Ru
Ruthenium
44
103
Rh
Rhodium
45
106
Pd
Palladium
46
108
Ag
Silver
47
112
Cd
Cadmium
48
115
In
Indium
49
119
Sn
Tin
50
122
Sb
Antimony
51
128
Te
Tellurium
52
127
I
Iodine
53
131
Xe
Xenon
54
137
Ba
Barium
56
139
La
Lanthanum
57*
178
Hf
Hafnium
72
181
Ta
Tantalum
73
184
W
Tungsten
74
186
Re
Rhenium
75
190
Os
Osmium
76
192
Ir
Iridium
77
195
Pt
Platinum
78
197
Au
Gold
79
201
Hg
Mercury
80
204
Tl
Thallium
81
207
Pb
Lead
82
209
Bi
Bismuth
83
Po
Polonium
84
At
Astatine
85
Rn
Radon
86
Fr
Francium
87
227
Ac
Actinium
89
9
Be
Beryllium
4
IIIIIIIVVVIVII0
85
Rb
Rubidium
37
133
Cs
Caesium
55
226
Ra
Radium
88
Thevolumeofonemoleofanygasis24dm3atroomtemperatureandpressure(r.t.p.).
a
X
b
a=relativeatomicmass
X=atomicsymbol
b=proton(atomic)number
Key
*58-71Lanthanoidseries
90-103Actinoidseries
DATASHEET
ThePeriodicTableoftheElements